Copyright © Houghton Mifflin Company. All rights reserved.4 | 1 Parts of Solutions Solution- homogeneous mixture. Solute- what gets dissolved. Solvent- what does the dissolving. Soluble- Can be dissolved. Miscible- liquids dissolve in each other.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 2 Figure 4.1 The Water Molecule

Copyright © Houghton Mifflin Company. All rights reserved.4 | 3 Hydration The process of breaking the ions of salts apart. Ions have charges and are attracted to the opposite charges on the water molecules.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 4 Figure 4.2 Polar Water Molecules Interact with the Positive and Negative Ions of a Salt Assisting in the Dissolving Process

Copyright © Houghton Mifflin Company. All rights reserved.4 | 5 How Ionic solids dissolve H H O H H O H H O H H O H H O H H O H H O H H O H H O Click here for Animation

Copyright © Houghton Mifflin Company. All rights reserved.4 | 6 Solubility How much of a substance will dissolve in a given amount of water. Usually g/100 mL Varies greatly, but if they do dissolve the ions are separated, and they can move around. Water can also dissolve non-ionic compounds if they have polar bonds.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 7 Figure 4.3a The Ethanol Molecule Contains a Polar O-H Bond Similar to Those in the Water Molecule

Copyright © Houghton Mifflin Company. All rights reserved.4 | 8 Figure 4.3b The Polar Water Molecule Interacts Strongly with the Polar-O-H bond in Ethanol

Copyright © Houghton Mifflin Company. All rights reserved.4 | 9 Electrolytes Electricity is moving charges. The ions that are dissolved can move. Solutions of ionic compounds can conduct electricity. Solutions are classified three ways.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 10 Types of solutions Strong electrolytes- completely dissociate (fall apart into ions). a)Many ions- Conduct well. Weak electrolytes- Partially fall apart into ions. a)Few ions -Conduct electricity slightly. Non-electrolytes- Don’t fall apart. a)No ions- Don’t conduct.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 11 Figure 4.4a-c Electrical Conductivity of Aqueous Solutions

Copyright © Houghton Mifflin Company. All rights reserved.4 | 12 Figure 4.5 NaCl Dissolves

Copyright © Houghton Mifflin Company. All rights reserved.4 | 13 Figure 4.6 HCL is Completely Ionized

Copyright © Houghton Mifflin Company. All rights reserved.4 | 14 Figure 4.7 An Aqueous Solution of Sodium Hydroxide

Copyright © Houghton Mifflin Company. All rights reserved.4 | 15 Figure 4.8 Acetic Acid (HC 2 H 3 O 2 )

Copyright © Houghton Mifflin Company. All rights reserved.4 | 16 Figure 4.9 The Reaction of NH 3 in Water

Copyright © Houghton Mifflin Company. All rights reserved.4 | 17 Measuring Solutions Concentration- how much is dissolved. Molarity = Moles of solute Liters of solution abbreviated M 1 M = 1 mol solute / 1 liter solution Calculate the molarity of a solution with 34.6 g of NaCl dissolved in 125 mL of solution.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 18 Figure 4.10a-c Steps Involved in the Preparation of a Standard Aqueous Solution

Copyright © Houghton Mifflin Company. All rights reserved.4 | 19 Figure 4.11a-b Measuring Pipets and Volumetric Pipets Measure Liquid Volume

Copyright © Houghton Mifflin Company. All rights reserved.4 | 20 Figure 4.12a-c A Measuring Pipet is Used to Add Acetic Solution to a Volumetric Flask

Copyright © Houghton Mifflin Company. All rights reserved.4 | 21 Figure 4.14 a&b Reactant Solutions

Copyright © Houghton Mifflin Company. All rights reserved.4 | 22 Figure 4.15 a&b The Reaction of K 2 CrO 4 and Ba(NO 3 ) 2

Copyright © Houghton Mifflin Company. All rights reserved.4 | 23 Figure 4.17 Molecular-Level Representations Illustrating the Reaction of KCl (aq) with AgNO 3 (aq) to Form AgCl (s)

Copyright © Houghton Mifflin Company. All rights reserved.4 | 24 Writing Net Ionic Equations Strong acids are all written in net ionic form -Binary acids – are all strong (except for HF (aq) ) -Oxyacids-If the number of oxygens exceeds the number of hydrogens by 2 or more they are considered strong. -Polyprotic acids ionize one (1) hydrogen at a time. All subsequent ionizations of acidic hydrogens are considered weak. (except for HSO 4(aq) 1- ) H 2 SO 4(aq) →H (aq) 1+ +HSO 4(aq) 1- Strong bases are all written in ionic form. -Group IA and IIA metal hydroxides are strong bases. All weak acids and bases (those not mentioned above) are always written in molecular form. Ionic Salts-If soluble-written in ionic form -if insoluble written in molecular/undissociated form.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 25 Writing Net Ionic Equations Oxides are always written in molecular/undissociated form. Gases are always written in molecular form. Molecular compounds are always written in molecular form.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 26 Determining the Mass of Product Formed

Copyright © Houghton Mifflin Company. All rights reserved.4 | 27 Determining the Mass of Product Formed

Copyright © Houghton Mifflin Company. All rights reserved.4 | 28 Performing Calculations for Acid-Base Reactions

Copyright © Houghton Mifflin Company. All rights reserved.4 | 29 Neutralization Reactions I

Copyright © Houghton Mifflin Company. All rights reserved.4 | 30

Copyright © Houghton Mifflin Company. All rights reserved.4 | 31

Copyright © Houghton Mifflin Company. All rights reserved.4 | 32

Copyright © Houghton Mifflin Company. All rights reserved.4 | 33

Copyright © Houghton Mifflin Company. All rights reserved.4 | 34

Copyright © Houghton Mifflin Company. All rights reserved.4 | 35 Neutralization Reactions II

Copyright © Houghton Mifflin Company. All rights reserved.4 | 36 Neutralization Titration

Copyright © Houghton Mifflin Company. All rights reserved.4 | 37 Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium Chloride

Copyright © Houghton Mifflin Company. All rights reserved.4 | 38 Figure 4.20 A Summary of Oxidation- Reduction Process

Copyright © Houghton Mifflin Company. All rights reserved.4 | 39 The Half-Reaction Method (Acidic Solution)

Copyright © Houghton Mifflin Company. All rights reserved.4 | 40 The Half-Reaction Method (Basic Solution)

Copyright © Houghton Mifflin Company. All rights reserved.4 | 41 Figure 4.4a-c Electrical Conductivity of Aqueous Solutions

Copyright © Houghton Mifflin Company. All rights reserved.4 | 42 An Aqueous Solution of Co(NO 3 ) 2.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 43 Figure 4.10 Steps Involved in the Preparation of a Standard Aqueous Solution

Copyright © Houghton Mifflin Company. All rights reserved.4 | 44 Figure 4.13 Yellow Aqueous Potassium

Copyright © Houghton Mifflin Company. All rights reserved.4 | 45 Figure 4.14a-b Reactant Solutions

Copyright © Houghton Mifflin Company. All rights reserved.4 | 46 Figure 4.15c Solution Post- Reaction

Copyright © Houghton Mifflin Company. All rights reserved.4 | 47 Figure 4.16 Addition of Silver Nitrate to Aqueous Solution of Potassium Chloride

Copyright © Houghton Mifflin Company. All rights reserved.4 | 48 Figure 4.17 Reaction of KCI(aq) with AgNO 3 (aq) to form AgCI(s).

Copyright © Houghton Mifflin Company. All rights reserved.4 | 49 Lead Sulfate

Copyright © Houghton Mifflin Company. All rights reserved.4 | 50 KOH and Fe(NO 3 ) 3 Mix to Create Solid Fe(OH) 3.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 51 Figure 4.18a-c The Titration of an Acid with a Base

Copyright © Houghton Mifflin Company. All rights reserved.4 | 52 Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium Chloride

Copyright © Houghton Mifflin Company. All rights reserved.4 | 53 Oxidation of Copper Metal by Nitric Acid

Copyright © Houghton Mifflin Company. All rights reserved.4 | 54 Magnetite

Copyright © Houghton Mifflin Company. All rights reserved.4 | 55 Aluminum and Iodine Mix to Form Aluminum Iodide

Copyright © Houghton Mifflin Company. All rights reserved.4 | 56 Chocolate

Copyright © Houghton Mifflin Company. All rights reserved.4 | 57 When Potassium Dichromate Reacts with Ethanol, the Solution Contains Cr 3+.

Copyright © Houghton Mifflin Company. All rights reserved.4 | 58 Table 4.1 Simple Rules for the Solubility of Salts in Water

Copyright © Houghton Mifflin Company. All rights reserved.4 | 59 Table 4.2 Rules for Assigning Oxidation States